Activation energy of a chemical reaction can be determined by

Half life of a first order reaction is 4 s and the initial concentration of the reactants is 0.12 M. The concentration of the reactant left after 16 s is

The plot of concentration of the reactant vs. time for a reaction is a straight line with a negative slope. The reaction follows a

Consider the reaction, 2A + B → products. When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is

Select the rate law that corresponds to data shown for the following reaction

The rate of reaction depends upon the

For a first order reaction (A) → products the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is :

The half -life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99 % of the chemical reaction will be (log 2 = 0.301)

The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be : (R = 8.314 JK–1 mol–1 and log 2 = 0.301)